AP Chemistry
6.9 Hess’s Law
6.6 Introduction to Enthalpy of Reaction
The combustion of carbon monoxide is represented by the thermochemical equation below:
\[ 2\,\text{CO}(g) + \text{O}_2(g) \rightarrow 2\,\text{CO}_2(g) \quad \Delta H^\circ = -560\text{ kJ/mol}_{\text{rxn}} \]
The equation is rewritten by multiplying all stoichiometric coefficients by a factor of \(2\):
\[ 4\,\text{CO}(g) + 2\,\text{O}_2(g) \rightarrow 4\,\text{CO}_2(g) \]
If a \(0.50\text{ mol}\) sample of \(\text{CO}(g)\) reacts completely with excess \(\text{O}_2(g)\), which of the following correctly gives the value of \(\Delta H^\circ\) for the rewritten equation and the quantity of heat released by the reaction of the sample?
\[ 2\,\text{CO}(g) + \text{O}_2(g) \rightarrow 2\,\text{CO}_2(g) \quad \Delta H^\circ = -560\text{ kJ/mol}_{\text{rxn}} \]
The equation is rewritten by multiplying all stoichiometric coefficients by a factor of \(2\):
\[ 4\,\text{CO}(g) + 2\,\text{O}_2(g) \rightarrow 4\,\text{CO}_2(g) \]
If a \(0.50\text{ mol}\) sample of \(\text{CO}(g)\) reacts completely with excess \(\text{O}_2(g)\), which of the following correctly gives the value of \(\Delta H^\circ\) for the rewritten equation and the quantity of heat released by the reaction of the sample?
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